Saint Patrick’s Bilingual School
Chemistry
Module 5: The Periodic Table and Periodic Law
Lesson 3. Periodic Trends
Name: _____________________________
Date: _____________________
Group: _____________________________
Points: ____________________
Directions: Use your notes and periodic table to answer the following questions.
1. Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen,
potassium. (4 pts.)
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2. Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum.
(4 pts.)
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3. Why does fluorine have a higher ionization energy than iodine? (3 pts.)
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4. Indicate whether the following properties increase or decrease from left to right across the
periodic table and top to bottom. (12 pts.)
a) atomic radius (excluding noble gases): ______________________________________.
b) ionization energy: _______________________________________________________.
c) electronegativity: _______________________________________________________.
5. Circle the atom in each pair that has the largest atomic radius. (6 pts.)
a) Al or B
b) Na or Al
c) S or O
d) O or F
e) Br or Cl
f) Mg or Ca
6.
Circle the atom in each pair that has the greater ionization energy. (5 pts.)
a) Li or Be
b) Ca or Ba
c) Na or K
d) P or Ar
e) Cl or Si
7.
Circle the atom in each pair that has the greater electronegativity. (6 pts.)
a) Ca or Ga
b) Br or As
c) Li or O
d) Ba or Sr
e) Cl or S
f) O or S
8. Using the periodic table, rank each group of elements in order of increasing size. (15 pts.)
a) calcium, magnesium, and strontium
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b) oxygen, lithium, and fluorine
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c) fluorine, cesium, and calcium
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d) selenium, chlorine, and tellurium
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e) iodine, krypton, and beryllium
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Increasing Electronegativity
Increasing Electronegativity